Answer:
a.
![Fe_2(SO_4)_3(aq)+6NaOH(aq)\rightarrow 2Fe(OH)_3(s)+3Na_2SO_4(aq)](https://tex.z-dn.net/?f=Fe_2%28SO_4%29_3%28aq%29%2B6NaOH%28aq%29%5Crightarrow%202Fe%28OH%29_3%28s%29%2B3Na_2SO_4%28aq%29)
b.
![2Fe^{2+}(aq)+3(SO_4)^{2-}(aq)+6Na^+(aq)+6OH^-(aq)\rightarrow 2Fe(OH)_3(s)+6Na^+(aq)+3(SO_4)^{2-}(aq)](https://tex.z-dn.net/?f=2Fe%5E%7B2%2B%7D%28aq%29%2B3%28SO_4%29%5E%7B2-%7D%28aq%29%2B6Na%5E%2B%28aq%29%2B6OH%5E-%28aq%29%5Crightarrow%202Fe%28OH%29_3%28s%29%2B6Na%5E%2B%28aq%29%2B3%28SO_4%29%5E%7B2-%7D%28aq%29)
c.
![Fe^{2+}(aq)+3OH^-(aq)\rightarrow Fe(OH)_3(s)](https://tex.z-dn.net/?f=Fe%5E%7B2%2B%7D%28aq%29%2B3OH%5E-%28aq%29%5Crightarrow%20Fe%28OH%29_3%28s%29)
Explanation:
Hello!
In this case, since the reaction between sodium hydroxide and iron (III) sulfate yields iron (III) hydroxide, an insoluble base, and sodium sulfate, a soluble salt, we can write the molecular equation as shown below:
a.
![Fe_2(SO_4)_3(aq)+6NaOH(aq)\rightarrow 2Fe(OH)_3(s)+3Na_2SO_4(aq)](https://tex.z-dn.net/?f=Fe_2%28SO_4%29_3%28aq%29%2B6NaOH%28aq%29%5Crightarrow%202Fe%28OH%29_3%28s%29%2B3Na_2SO_4%28aq%29)
Now, for the total ionic equation, we make sure we separate the aqueous species in ions (dissociation) in order to write:
b.
![2Fe^{2+}(aq)+3(SO_4)^{2-}(aq)+6Na^+(aq)+6OH^-(aq)\rightarrow 2Fe(OH)_3(s)+6Na^+(aq)+3(SO_4)^{2-}(aq)](https://tex.z-dn.net/?f=2Fe%5E%7B2%2B%7D%28aq%29%2B3%28SO_4%29%5E%7B2-%7D%28aq%29%2B6Na%5E%2B%28aq%29%2B6OH%5E-%28aq%29%5Crightarrow%202Fe%28OH%29_3%28s%29%2B6Na%5E%2B%28aq%29%2B3%28SO_4%29%5E%7B2-%7D%28aq%29)
Finally, the net ionic equation comes up by cancelling out the spectator ions, those at both reactants and products sides:
![2Fe^{2+}(aq)+6OH^-(aq)\rightarrow 2Fe(OH)_3(s)](https://tex.z-dn.net/?f=2Fe%5E%7B2%2B%7D%28aq%29%2B6OH%5E-%28aq%29%5Crightarrow%202Fe%28OH%29_3%28s%29)
Or just:
c.
![Fe^{2+}(aq)+3OH^-(aq)\rightarrow Fe(OH)_3(s)](https://tex.z-dn.net/?f=Fe%5E%7B2%2B%7D%28aq%29%2B3OH%5E-%28aq%29%5Crightarrow%20Fe%28OH%29_3%28s%29)
Best regards!
Crystals of phthalic acid can be grown twice as fast compared to the smaller crystals
LMBO, for science.
Answer:
<em>The increase in kinetic energy leads to leakage of water from the syringe. When the outside temperature is more than the liquid temperature, say the syringe is out in sunshine, then the liquid becomes slightly warmer.</em>
Molar mass of cuso4=63.5+32+4*16= 159.5 g
6.02*10^23 molecules weigh=159.5 g
1 molecule weigh=159.5/6.02*10^23 g
3.36 × 10^23 molecules weigh=159.5/6.02*10^23*3.36× 10^23
=89.023g
Given the number of Mg atoms is ![7.43 * 10^{22} atoms](https://tex.z-dn.net/?f=%207.43%20%2A%2010%5E%7B22%7D%20atoms%20%20)
We know that 1 mol of any substance has Avogadro number
of formula units.
Converting number of atoms to mol:
![7.43 * 10^{22} atoms * \frac{1 mol}{6.022*10^{23} atoms} = 0.123 mol Mg](https://tex.z-dn.net/?f=%207.43%20%2A%2010%5E%7B22%7D%20atoms%20%2A%20%5Cfrac%7B1%20mol%7D%7B6.022%2A10%5E%7B23%7D%20atoms%7D%20%20%20%3D%200.123%20mol%20Mg%20)
Converting mol to mass of Mg:
![0.123 mol * \frac{24.30 g}{1 mol} = 2.99 g Mg](https://tex.z-dn.net/?f=%200.123%20mol%20%2A%20%5Cfrac%7B24.30%20g%7D%7B1%20mol%7D%20%3D%202.99%20g%20Mg%20)
Therefore mass of Mg is <u>2.99 g</u>